- A 445 g sample of ice at –58oC is heated until its temperature reaches –29oC. Find the change in heat content of the system.
- A 152 g sample of ice at –37oC is heated until it turns into liquid water at 0oC. Find the change in heat content of the system.
- A 218 g sample of steam at 121oC is cooled to ice at –14oC. Find the change in heat content of the system.
- If 161 g of water at 85oC is cooled to ice at 0oC, find the change in heat content of the system.
- A 79 g sample of water at 21oC is heated until it becomes steam with a temperature of 143oC. Find the change in heat content of the system.
- If a 348 g sample of steam at 127oC is cooled to 103oC, find the change in heat content of the system.
- In going from ice at –34oC to steam at 138oC, a sample of water absorbs 1.41 x 105 J. Find the mass of the sample.
- You find a penny in the snow. How much heat is absorbed by the penny as it warms from the temperature of the snow, which is -8.0oC, to the temperature of your body, 37oC? Assume the penny is pure copper and has a mass of 31.0 g. Use the information from question #14 for the specific heat of copper.
- Consider the following specific heats of metals.
Metal Specific Heat
copper 0.385 J/(g • °C)
cobalt 0.418 J/(g • °C)
chromium 0.447 J/(g • °C)
gold 0.129 J/(g • °C)
silver 0.237 J/(g • °C)If 100-g samples of each of the metals at 95°C are added to 100 mL of water at 25°C. Which element from the table increase the temperature of the water the greatest amount? - The specific heat capacity of methane gas is 2.20 J/g-°C. How many joules of heat are needed to raise the temperature of 5.00 g of methane from 36.0°C to 75.0°C?
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The change in heat content of the system.
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